8.1 Names of Atoms Chapter 8 Nomenclature Simple neutral atoms with no charge are named as is: Na is sodium atom, Ne is neon atom Know the names and symbols for elements #1-20 and Ba, Co, I, Cu, Fe, Pb, Hg, Ag, Au, Zn, Sn, Sr, Ni, Br, Cr, Mn, Cd Ba barium Co cobalt I iodine Zn zinc Br bromine Cd cadmium Cu copper Fe iron Pb lead Sn tin Cr chromium Sr strontium Hg mercury Ag silver Au gold Ni nickel Mn manganese Definitions: ionic compound: metal + nonmetal(s) (eg. NaCl, CaBr 2, KMnO 4, BaSO 4 ) covalent compound: 2 or more nonmetals (eg. NH 3, CCl 4 ) monoatomic ion: charged ion from a single atom (eg Na +, Cl, O 2 ) polyatomic ion: charged ion containing 2 or more atoms (eg. OH, SO 4 2 ) Oxidation States Oxidation state is a fancy name for charge o All elements alone have a charge of zero in their elemental state o Atoms get a charge and become ions when they have lost or gained electrons CATIONS - positively charged ion resulting from a neutral metal atom losing one or more e- s. Fixed Charge The charge is always the same value based on electron configuration. Typically group A representative metals. Group IA metals always have a +1 charge when they become an ion. Example: Na + is sodium ion, K + is potassium ion Group IIA metals always have a +2 charge when they become an ion. Example: Mg 2+ is magnesium ion, Sr 2+ is strontium ion Ion Charge Roman Numeral +1 I +2 II +3 III +4 IV +5 V +6 VI Group IIIA metals always have a +3 charge when they become an ion. Example: Al 3+ is aluminum ion, Ga 3+ is gallium ion Exceptions: The transition metals Ag +1, Zn 2+, and Cd 2+ have fixed charges. Variable Charge The charge can be a different value based on oxidation state. Typically group B transition metals. Use a Roman Numeral to indicate the charge of the cation if there is more than one possible charge. Clark, Smith (CC-BY-SA 4.0) GCC CHM 130 Chapter 8: Nomenclature page 1
Example: Fe can have two oxidation states Fe 2+ is iron (II) ion Fe 3+ is iron (III) ion Exceptions: Group A metals Sn and Pb Sn 2+ is tin (II) ion, Sn 4+ is tin (IV) ion Pb 2+ is lead (II) ion, Pb 4+ is lead (IV) ion ANIONS negatively charged ion resulting from a neutral nonmetal atom gaining one or more e - s. Monatomic anions: Name changes for these anions by adding ide ending. Always a fixed charged - based on electron configuration Group VA gain 3 e - s to make 3- ions. N 3- nitride ion P 3- phosphide ion O atom: [He] 2s 2p Group VIA gain 2 e - s to make 2- ions O 2- oxide ion O 2- ion: [He] S 2- sulfide ion 2s 2p Group VIIA gain 1 e - to make 1- ions F - fluoride ion Cl - chloride ion Br - bromide ion I - iodide ion Oxygen gains only two electrons. The resulting oxide ion is then isoelectronic to the noble gas neon, Ne. POLYATOMICS two or more nonmetals covalently bonded with an overall charge. Here is the complete list of Polyatomic Ions you are responsible for this semester: NH 4 + = ammonium Most Common Polyatomic Ions C 2 H 3 O 2 - = acetate OH - = hydroxide CN - = cyanide MnO 4 - = permanganate CO 3 2- = carbonate HCO 3 - = hydrogen carbonate or bicarbonate NO 3 - = nitrate NO 2 - = nitrite SO 4 2- = sulfate SO 3 2- = sulfite PO 4 3- = phosphate CrO 4 2- = chromate Cr 2 O 7 2- = dichromate *These are given to you on your CHM130 Periodic Table for quizzes and exams. 8.2 Ionic Formulas Compounds are Neutral They have no net charge so you must have enough cations and anions to equal zero. Na + and Cl make NaCl since +1 and 1 = 0 Na + and CN make NaCN since +1and 1 = 0 Ba 2+ and Cl make BaCl 2 since +2 and 2(-1) = 0 Clark, Smith (CC-BY-SA 4.0) GCC CHM 130 Chapter 8: Nomenclature page 2
Al 3+ and O 2 make Al 2 O 3 since 2(+3) and 3(-2) = 0 Cu(II) and Br make CuBr 2 since +2 and 2(-1) = 0 Polyatomic ions are just the same, remember to keep them together as a group Express more than one polyatomic ion with subscripts and parentheses. Sr 2+ and NO 3 - make Sr(NO 3 ) 2 since +2 and 2(-1) = 0 Fe 3+ and CO 3 2 make Fe 2 (CO 3 ) 3 since 2(+3) and 3(-2) = 0 8.3 Ionic Names The name is always the cation (usually metal) first then the anion + -ide ending. Fixed Charge Metal: metal name + nonmetal name + ide Variable Charge Metal: metal name (charge of metal) + nonmetal name + ide Don t change the name for polyatomic ions to end in ide. For variable charge metals use a Roman Numeral to indicate the metal s charge. How do you figure out the charge on a variable charge metal? Well you look at the anion s charge. Cu(OH) 2 Cu(OH) 2 OH- OH- The subscript of 2 indicates there are 2 OH - ions in the formula. Cu 2+ The overall compound has zero charge, so the Cu ion must be 2+ to cancel the two -1 charges from the two hydroxide ions present. Given the formula of a compound, predict the name: What is the name for NaCl? sodium chloride (no Roman # since know Na is +1) What is the name for K 2 SO 4? potassium sulfate (keep the polyatomic name as is) What is the name for CuCl? copper (I) chloride since Cl is 1 so Cu must be +1 What is the name for FePO 4? iron (III) phosphate since PO 4 is 3 so Fe must be +3 Name for Ca(NO 3 ) 2? calcium nitrate Name for Na 2 O? sodium oxide Note: Never capitalize the names of compounds! Given the name of a compound, predict the formula: You must know charges on ions formed by Group A main elements. Know how to use polyatomic ions given on your Periodic Table! lithium sulfide Li 2 S since Li is +1 and S is 2 you need two Li s calcium oxide CaO since Ca is +2 and O is 2 you just need one of each iron (II) bromide FeBr 2 since Fe is +2 and Br is 1 you need two Br s potassium acetate KC 2 H 3 O 2 since K is +1 and acetate is 1, need one of each gold (II) nitrite Au(NO 2 ) 2 since Au is +2 and NO 2 is 1, need two nitrites sodium iodide NaI since Na is +1 and I is 1, just need one of each Clark, Smith (CC-BY-SA 4.0) GCC CHM 130 Chapter 8: Nomenclature page 3
8.4 Covalent Names Molecular Compounds: compounds consisting of 2 nonmetals. These are NOT ions, so no charges. You are not trying to add up to zero charge with these. Number of atoms of element indicated by Greek prefix before element name FIRST ELEMENT prefix (except mono) + nonmetal name # of atoms Greek prefix # of atoms Greek prefix 1 mono 6 hexa 2 di 7 hepta 3 tri 8 octa 4 tetra 9 nona 5 penta 10 deca Examples: CO 2 = carbon dioxide PCl 3 = phosphorus trichloride N 2 S 5 = dinitrogen pentasulfide SF 6 = sulfur hexafluoride Cl 2 O 7 = dichlorine heptaoxide SECOND ELEMENT prefix + 2 nd nonmetal name + ide 2 nitrogen atoms = di N 2 O 4 4 oxygen atoms = tetra dinitrogen tetraoxide or dinitrogen tetroxide Prefixes are ONLY used with molecular compounds. Roman numerals are ONLY used with variable charged metal ionic compounds. Polyatomic ions never change their name. CHAPTER 8 PRACTICE PROBLEMS Example 1: Example 2: Circle all the examples below that are ionic compounds. Circle all the examples below that are covalent compounds. Clark, Smith (CC-BY-SA 4.0) GCC CHM 130 Chapter 8: Nomenclature page 4
Example 3: What ions are the following atoms most likely to make? calcium = potassium = sulfur = aluminum = nitrogen = chlorine = silver = zinc = Example 4: What is the name for: CuCl 2, SrS, NiCrO 4, Mg(NO 3 ) 2, Na 3 P, ZnCO 3, KOH, Ca(CN) 2 Example 5: What is the formula for sodium carbonate, copper(ii) bromide, strontium fluoride, iron(iii) nitride, silver sulfite, nickel(ii) nitrate, cadmium phosphate, ammonium hydroxide, magnesium sulfate? Example 6: What is the name for CF 4, CO, PO 5, N 2 F 4? What is the formula for diphosphorus tetraiodide, tribromine octaoxide, tetraphosphorus decasulfide, carbonic acid? Answers to Practice Problems Example 1: Circle all the examples below that are ionic compounds. metal-nonmetal Example 2: Circle all the examples below that are molecular compounds. nonmetals Example 3: calcium = Ca 2+ potassium = K + sulfur = S 2- aluminum = Al 3+ nitrogen = N 3- chlorine = Cl - silver = Ag + zinc = Zn 2+ Example 4: CuCl 2 SrS NiCrO 4 Mg(NO 3 ) 2 ZnCO 3 Na 3 P KOH Ca(CN) 2 name copper(ii) chloride strontium sulfide nickel(ii) chromate magnesium nitrate zinc carbonate sodium phosphide potassium hydroxide calcium cyanide Example 5: formula sodium carbonate Na 2 CO 3 copper(ii) bromide CuBr 2 strontium fluoride SrF 2 iron(iii) nitride FeN silver sulfite Ag 2 SO 3 nickel(ii) nitrate Ni(NO 3 ) 2 cadmium phosphate Cd 3 (PO 4 ) 2 ammonium hydroxide NH 4 OH magnesium sulfate MgSO 4 Example 6: carbon tetrafluoride, carbon monoxide, phosphorus pentaoxide, dinitrogen tetrafluoride, P 2 I 4, Br 3 O 8, P 4 S 10, H 2 CO 3 Clark, Smith (CC-BY-SA 4.0) GCC CHM 130 Chapter 8: Nomenclature page 5